Balance the following redox reaction if it occurs in acidic solution. What are t

Question

Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of Sn and Ag^+ in the balanced reaction? Sn(s) + Ag^+(aq) rightarrow Ag(s) + Sn^2+(aq) Sn = 1, Ag^* = 2 Sn = 1, Ag^* = 1 Sn = 2, Ag^* = 1 Sn = 2, Ag^* = 2 Sn = 3, Ag* = 1 A galvanic cell consists of one half-cell that contains Ag(s) and Ag^+(aq); and one half-cell that contains Cu(s) and Cu^2+(aq). What species are produced at the electrodes under standard conditions? Ag^+ (aq) + e^- rightarrow Ag(s) E degree = +0.80 V Cu^2+(aq) + 2e^- rightarrow Cu(s) E degree = +0.34 V Ag(aq) is formed at the cathode and, Cu(s) is formed at the anode. Ag(s) is formed at the cathode, and Cu^2+(aq) is formed at the anode. Cu(s) is formed at the cathode, and Ag^+(aq) is formed at the anode. Cu^2+(aq) is formed at the cathode, and Cu(s) is formed at the anode.

Explanation / Answer

24)

Sn + Ag+ -----------------> Sn 2+ + Ag

oxidation : Sn ------------> Sn 2+ + 2e-

reduction : 2Ag+ + 2e- ------------------> 2Ag

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overall reaction : Sn + 2Ag+ ----------------> Sn 2+ + 2Ag

25)

anode : Cu -------------> Cu+2 + 2e-    Eo = 0.34 V

cathode : 2Ag+ + 2e-   ----------------> 2Ag (s)      Eo = 0.80 V.

here

reduction potential of Cu is less . so it is anode . and the reduction potential of Ag is higher. so it is cathode.

so Ag(s) formed at cathode

Cu+2 formed at anode

so option b) is correct

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